Exploring Probenecid Derived 1,3,4-Oxadiazole-Phthalimide Hybrid as α-Amylase Inhibitor: Synthesis, Structural Investigation, and Molecular Modeling

1,3,4-Oxadiazole moiety is a crucial pharmacophore in many biologically active compounds. In a typical synthesis, probenecid was subjected to a sequence of reactions to obtain a 1,3,4-oxadiazole–phthalimide hybrid (PESMP) in high yields. The NMR (1H and 13C) spectroscopic analysis initially confirmed the structure of PESMP. Further spectral aspects were validated based on a single-crystal XRD analysis. Experimental findings were confirmed afterwards by executing a Hirshfeld surface (HS) analysis and quantum mechanical computations. The HS analysis showed the role of the π⋯π stacking interactions in PESMP. PESMP was found to have a high stability and lower reactivity in terms of global reactivity parameters. α-Amylase inhibition studies revealed that the PESMP was a good inhibitor of α-amylase with an s value of 10.60 ± 0.16 μg/mL compared with that of standard acarbose (IC50 = 8.80 ± 0.21 μg/mL). Molecular docking was also utilized to reveal the binding pose and features of PESMP against the α-amylase enzyme. Via docking computations, the high potency of PESMP and acarbose towards the α-amylase enzyme was unveiled and confirmed by docking scores of −7.4 and −9.4 kcal/mol, respectively. These findings shine a new light on the potential of PESMP compounds as α-amylase inhibitors.


Introduction
Diabetes mellitus is a chronic disease aroused by the inability of the body to consume blood sugar, which leads to high blood sugar levels and the malfunction of the vascular system, vision, urinary system, and nerves. According to a WHO report, about 422 million people all around the globe are suffering from diabetes mellitus and 1.5 million/year deaths are caused by it; an ascending trend in these numbers has been continuously observed [1,2]. α-Amylase is released by the salivary glands and pancreas and catalyzes the breakdown of starch and polysaccharides to produce sugars as end-products. The excessive production of this enzyme causes an accelerated degradation of polysaccharides, resulting in an extreme sugar concentration in the blood. One way to control diabetes mellitus is to control the release of α-amylase in the blood, thus producing a restricted amount of sugars [3].

Introduction
Diabetes mellitus is a chronic disease aroused by the inability of the body to consume blood sugar, which leads to high blood sugar levels and the malfunction of the vascular system, vision, urinary system, and nerves. According to a WHO report, about 422 million people all around the globe are suffering from diabetes mellitus and 1.5 million/year deaths are caused by it; an ascending trend in these numbers has been continuously observed [1,2]. α-Amylase is released by the salivary glands and pancreas and catalyzes the breakdown of starch and polysaccharides to produce sugars as end-products. The excessive production of this enzyme causes an accelerated degradation of polysaccharides, resulting in an extreme sugar concentration in the blood. One way to control diabetes mellitus is to control the release of α-amylase in the blood, thus producing a restricted amount of sugars [3]. 1,3,4-Oxadiazole, a five-membered heterocycle moiety with two nitrogen atoms and one oxygen atom in the cycle, has been recognized to have a decreased aromatic and improved diene character [4]. Compounds relevant to this category of heterocycles have expressed a versatile therapeutic potential as antimicrobial [5], antiepileptic [6], anticancer [7,8], hypoglycemic [9,10], antiviral [11], and anti-inflammatory agents ( Figure 1) [12]. Many commercially available drugs bear the 1,3,4-oxadiazole moiety in their core structure as a pharmacophore ( Figure 1) [13]. Among those drugs, raltegravir is used to treat HIV [14], furamizole treats microbial infections [15], nesapidil is prescribed as a vasodilator [16], and zibotentan is an anticancer drug [17]. The developments in the synthesis of 1,3,4-oxadiazole scaffolds and their biological activities have been reviewed [18,19]. Probenecid, a sulfonamide containing benzoic acid, is a commercially available drug used to manage hyperuricemia [20]. Probenecid-derived amide linkage-containing structures have been successfully synthesized and analyzed for their carbonic anhydrase inhibition [21]. A little less attention has been devoted to the conversion of probenecid into its oxadiazole derivatives and investigations of their biological activities. However, probenecid-derived 1,3,4-oxadiazole-phthalimide hybrids have been investigated for their dengue virus NS2B/NS3 protease inhibition [10]. Moreover, phthalimide-based 1,3,4-oxadiazoles have been found to be anticonvulsant [22], cytotoxic [23], and peripheral analgesic [24] agents. In the context of our previous research [10,25], we envisioned that a combination of probenecid, 1,3,4-oxadiazole, and phthalimide moieties to access a hybrid molecule might result in enhancing enzyme inhibitions. Thus, a synthesis of enzyme inhibitors was undertaken, along with a single-crystal analysis, DFT exploration, and α-amylase inhibition studies of probenecid-derived 1,3,4oxadiazole-phthalimide hybrids. Docking predictions were carried out to unveil the docking pose and score of PESMP against the α-amylase enzyme. These findings shine new light on the potential of PESMP as an α-amylase inhibitor.

Chemistry
The PESMP compound was synthesized by a multi-step synthetic path, as depicted in Scheme 1. The purity of PESMP was confirmed based on thin-layer chromatography. The pure compound had a melting point of 154-155 • C. In the 1 H NMR spectrum of PESMP ( Figure S1), a triplet at δ 0.89 ppm (coupling constant = 7.35 Hz) was designated for six protons. A multiplet for four protons of two methylene groups (CH 3 CH 2 CH 2 ) was observed at δ 1.49-1.66 ppm. Another multiplet for four protons of two methylene groups (N-CH 2 ) attached to the N-atom was present at δ 3.00-3.22 ppm. A singlet for two protons at δ 5.41 ppm represented SCH 2 N. The aromatic protons were detected between δ 7.71 and 8.25 ppm.
The molecules are further connected via C-H···O bonding to form R 2 2 (10) hydrogenbonded loops ( Figure 4). The R 2 2 (10) H-bonded loops are connected through C-H· · · O and C-H· · · N bonding. As a result, R 2 2 (8) H-bonded loops are formed. The weak intramolecular π· · · π stacking interactions are unveiled via crystal packing. The five-membered ring of group A is involved in an intra-molecular π· · · π stacking interaction with the five-membered ring of group B with an inter-centroid separation value of 4.08 Å (Figure 4). The dihedral angle between the rings is 26.27(8) • . bonded loops (Figure 4). The R (10) H-bonded loops are connected through C-H⋯O and C-H⋯N bonding. As a result, R (8) H-bonded loops are formed. The weak intra-molecular π⋯π stacking interactions are unveiled via crystal packing. The five-membered ring of group A is involved in an intra-molecular π⋯π stacking interaction with the five-membered ring of group B with an inter-centroid separation value of 4.08 Å ( Figure 4). The dihedral angle between the rings is 26.27(8) °. The inter-centroid separation of the intermolecular offset π⋯π stacking interactions is observed in the range of 3.33-3.72 Å, forming a chain of molecules along the [110] direction. The similar five-membered rings of the symmetry-related molecules are involved in inter-molecular offset π⋯π stacking interactions with the ring offset, or slippage ranges from 1.396 to 1.994 Å. The CH from one of the propyl groups participates in the C-H⋯π interaction with the aromatic ring of the symmetry-related molecules (1+x, y, z), which forms an infinite chain of molecules that goes along the a-axis ( Figure 5a, Table 2). An intra-molecular C-O ⋯ π interaction is found in PESMP with an O ⋯ π distance of The inter-centroid separation of the intermolecular offset π· · · π stacking interactions is observed in the range of 3.33-3.72 Å, forming a chain of molecules along the [110] direction. The similar five-membered rings of the symmetry-related molecules are involved in inter-molecular offset π· · · π stacking interactions with the ring offset, or slippage ranges from 1.396 to 1.994 Å. The CH from one of the propyl groups participates in the C-H· · · π interaction with the aromatic ring of the symmetry-related molecules (1 + x, y, z), which forms an infinite chain of molecules that goes along the a-axis ( Figure 5a, Table 2). An intramolecular C-O· · · π interaction is found in PESMP with an O· · · π distance of 3.2430 (12) • and a C-O· · · π angle of 90.74(9) • [26]. In crystal packing, the inter-molecular C-O· · · π interaction shows an O· · · π distance of 3.2417 (12) Å and a C-O· · · π angle of 80.93(8) • , which interlink the molecules in the form of dimers ( Figure 5b, Table 2).  Table 2).

Hirshfeld Surface Analysis and Interaction Energy Calculation
A Hirshfeld surface (HS) analysis is an informative technique to elaborate and recognize non-covalent interactions in single crystals. It was developed to divide crystal densi- Figure 5. Representation for (a) C-H· · · π interactions that form an infinite chain of molecules besides the a-axis, (b) C-O· · · π interactions that interlink molecules through a dimeric form. Distances are in Å.

Hirshfeld Surface Analysis and Interaction Energy Calculation
A Hirshfeld surface (HS) analysis is an informative technique to elaborate and recognize non-covalent interactions in single crystals. It was developed to divide crystal densities into molecular fragments [27][28][29][30][31][32][33]. The hydrogen bonding interactions can be elucidated using HS plots over the normalized distance (d norm ) property. The red-and blue-colored regions on surface stand for short and long contacts, respectively. Meanwhile, the spots on the white region indicate that the contacts have distances between their atoms equal to the sum of the van der Waals radii summation. Figure 6a,b show the HS surfaces over normalized distances (d norm ) and shape index, respectively. Figure 5. Representation for (a) C-H⋯π interactions that form an infinite chain of molecules besides the a-axis, (b) C-O⋯π interactions that interlink molecules through a dimeric form. Distances are in Å.

Hirshfeld Surface Analysis and Interaction Energy Calculation
A Hirshfeld surface (HS) analysis is an informative technique to elaborate and recognize non-covalent interactions in single crystals. It was developed to divide crystal densities into molecular fragments [27][28][29][30][31][32][33]. The hydrogen bonding interactions can be elucidated using HS plots over the normalized distance (dnorm) property. The red-and bluecolored regions on surface stand for short and long contacts, respectively. Meanwhile, the spots on the white region indicate that the contacts have distances between their atoms equal to the sum of the van der Waals radii summation. Figures 6a and 6b show the HS surfaces over normalized distances (dnorm) and shape index, respectively.  The red spots around one of the O-atoms of the carbonyl and sulfonyl groups as well as the one N-atom of the 2,5-dihydro-1,3,4-oxadiazole confirm the contributions of the H-bonding interactions (Figure 6a). The interactions of π· · · π stacking can be recognized by extracting the HS over the shape index property. The occurrence of successive blue and red triangular patches on the HS around the aromatic ring shows π· · · π stacking interactions [34]. These areas are noted on the HS plots relevant to the shape index property for PESMP (Figure 6b), which confirms the existence of π· · · π stacking interactionsin PESMP. The contribution of the interatomic contacts in defining the overall packing of the crystal is determined by a 2D fingerprint plot analysis [25,[35][36][37][38][39]. 2D fingerprints of all the interactions are generated (Figure 7). The reciprocal contacts are also included while forming the 2D plots.
Overall interaction is displayed in Figure 7a. The most significant contributor to crystal packing is announced to be the H· · · H contact, with 35.3% (Figure 7b). The other important contacts are O· · · H, C· · · H, N· · · H, and S· · · H, with contributions of 35.3%, 28.1%, 14%, 6.6%, and 6.1%, respectively (Figure 7c-f). The C· · · C and C· · · N contacts show lower contributions to the crystal packing as compared to the contacts, as shown in Figure 7, although these contacts are involved in π· · · π stacking interactions. The contacts that have comparatively smaller percentage contributions to the crystal packing are shown in Figure S3.
The enrichment ratio provides the actual contacts for a given single crystal [40,41]. The enrichment ratio is determined as a result of the division of the actual contact value obtained directly from CrystalExplorer by the ratio of the random contact determined theoretically. The enrichment ratio values for the pair of chemical species are summarized in Table 3. red triangular patches on the HS around the aromatic ring shows π⋯π stacking interactions [34]. These areas are noted on the HS plots relevant to the shape index property for PESMP (Figure 6b), which confirms the existence of π⋯π stacking interactionsin PESMP. The contribution of the interatomic contacts in defining the overall packing of the crystal is determined by a 2D fingerprint plot analysis [25,[35][36][37][38][39]. 2D fingerprints of all the interactions are generated (Figure 7). The reciprocal contacts are also included while forming the 2D plots. Overall interaction is displayed in Figure 7a. The most significant contributor to crystal packing is announced to be the H⋯H contact, with 35.3% (Figure 7b). The other important contacts are O⋯H, C⋯H, N⋯H, and S⋯H, with contributions of 35.3%, 28.1%, 14%, 6.6%, and 6.1%, respectively (Figure 7c-f). The C⋯C and C⋯N contacts show lower contributions to the crystal packing as compared to the contacts, as shown in Figure 7, although these contacts are involved in π⋯π stacking interactions. The contacts that have comparatively smaller percentage contributions to the crystal packing are shown in Figure  S3.
The enrichment ratio provides the actual contacts for a given single crystal [40,41]. The enrichment ratio is determined as a result of the division of the actual contact value obtained directly from CrystalExplorer by the ratio of the random contact determined theoretically. The enrichment ratio values for the pair of chemical species are summarized in Table 3.  According to the compiled data in Table 3, C· · · C was the most favorable contact with an enrichment ratio of 3.31. The second most favorable contact was O· · · H, with an enrichment ratio of 1.39. The H· · · H and C· · · C contacts became less favorable by decreasing the enrichment ratio to less than one. A possible reason for the higher enrichment ratio of the C· · · N contact as compared to that of the C· · · C contact is that the intermolecular offset π· · · π stacking and C-O· · · π interaction interactions involve π-rings containing one or more nitrogen atoms. In crystal packing, various features of the single crystals, especially their mechanical properties, depending on the voids. For a single crystal to have good mechanical properties, the voids should be small. The voids were assessed by means of the Hartree-Fock theory, and the electronic densities of all the atoms were added up by supposing the spherical nature of the atoms [42][43][44][45][46]. Figure S4 is the graphical view of the voids in PESMP. The volume of voids was 148.35 Å 3 , which indicated that only 12.6% of the total volume was taken up by voids. The void research addressed the tight packing of molecules along with the lack of significant cavities in the crystal packing of the PESMP compound.
The CrystalExplorer software was employed for the calculation of the interaction energy within the molecular pairs. The calculation was carried out on a series of molecules located within 3.8 Å 3 of the reference molecule using the B3LYP/6-31G(d,p) computational level. The symmetry-related molecules are displayed in Figure 8a. The obtained findings of the interaction energies among the molecular pairs are shown in Table S2. Table S3 collects the utilized atomic coordinates in the interaction energy calculations. As summarized in Table S2, the highest attractive total energy was for the pair of molecules with an intermolecular distance of 8.14 Å. The highest energy value of -92.7 kJ/mol reflected attractive forces, indicating that the molecules were connected by inversion symmetry. The lowest attractive total energy with a value of -7.1 kJ/mol was found for the molecular pair with a distance of 19.10 Å between molecular centroids. For only one molecular pair, the total interaction energy was repulsive, with a value of 0.2 kJ/mol. Electrostatic energy was attractive for most of the molecular pairs except for the molecular pair R = 12.91 Å.
Figures 8b-d show the energy framework for coulomb, dispersion and total energy, respectively. The molecular centers were attached by the cylinders, and the thickness of the cylinder was directly related to the interaction strength. For the electrostatic coulomb energy, the thickness of the cylinders (Figure 8b) was smaller than that for the dispersion energy (Figure 8c), indicating that the dispersion energy was dominant over the coulomb energy. As summarized in Table S2, the highest attractive total energy was for the pair of molecules with an intermolecular distance of 8.14 Å. The highest energy value of −92.7 kJ/mol reflected attractive forces, indicating that the molecules were connected by inversion symmetry. The lowest attractive total energy with a value of −7.1 kJ/mol was found for the molecular pair with a distance of 19.10 Å between molecular centroids. For only one molecular pair, the total interaction energy was repulsive, with a value of 0.2 kJ/mol. Electrostatic energy was attractive for most of the molecular pairs except for the molecular pair R = 12.91 Å. Figure 8b-d show the energy framework for coulomb, dispersion and total energy, respectively. The molecular centers were attached by the cylinders, and the thickness of the cylinder was directly related to the interaction strength. For the electrostatic coulomb energy, the thickness of the cylinders (Figure 8b) was smaller than that for the dispersion energy (Figure 8c), indicating that the dispersion energy was dominant over the coulomb energy.

DFT Calculations 2.4.1. Frontier Molecular Orbitals Analysis
Frontier molecular orbitals (FMOs) theory is employed as a dependable tool for estimating the electronic properties along with the chemical stability of a system [47,48]. In the context of FMOs, the electron density distribution in molecular orbitals is elucidated. FMOs also interpret the chemical affinity and relation of the examined molecule with other moieties. Furthermore, FMOs support our understanding of the reactive sites in any π-electron system [49]. FMOs investigate two principal orbitals. The first one is the highest occupied molecular orbital (HOMO), which holds and donates electrons as an electron donor. The second one is the lowest unoccupied molecular orbital (LUMO), which has a vacant orbital and tends to receive electrons [50]. Via E HOMO and E LUMO values, the FMO's band gap (∆E) is computed to elucidate the reactivity, electron transference properties, hardness, and softness of a molecule. The compounds possessing a greater energy difference between HOMO and LUMO are considered to be harder, kinetically more stable, and less reactive in their nature and vice versa [51].
For the PESMP compound, FMO calculations were carried out, and the results of HOMO, HOMO − 1, HOMO − 2, LUMO, LUMO + 1, and LUMO + 2, along with their corresponding band gaps, are collected in Table 4. The molecular orbital sketch of the PESMP compound is shown in Figure 9. Frontier molecular orbitals (FMOs) theory is employed as a dependable tool for estimating the electronic properties along with the chemical stability of a system [47,48]. In the context of FMOs, the electron density distribution in molecular orbitals is elucidated. FMOs also interpret the chemical affinity and relation of the examined molecule with other moieties. Furthermore, FMOs support our understanding of the reactive sites in any π-electron system [49]. FMOs investigate two principal orbitals. The first one is the highest occupied molecular orbital (HOMO), which holds and donates electrons as an electron donor. The second one is the lowest unoccupied molecular orbital (LUMO), which has a vacant orbital and tends to receive electrons [50]. Via EHOMO and ELUMO values, the FMO's band gap (ΔE) is computed to elucidate the reactivity, electron transference properties, hardness, and softness of a molecule. The compounds possessing a greater energy difference between HOMO and LUMO are considered to be harder, kinetically more stable, and less reactive in their nature and vice versa [51].
In the PESMP compound, the charge density for HOMO was found over the oxadiazole and benzenesulfonamide moieties (Figure 9). The charge density for LUMO was situated on the phthalimide moiety, predicting an excellent charge transference from oxadiazole and benzenesulfonamide toward the phthalimide moiety.
The chemical hardness (η) of a molecule is related to the energy gap (∆E) value. The overall softness and reactivity of the PESMP compound demonstrated an inverse relationship. η showed a value of 0.0866 a.u., revealing the high stability and lower reactivity of the considered compound. The ionization potential (IP) and electron affinity (EA) values were 0.2678 and 0.0946 a.u., respectively. Moreover, the values of µ, ω, and σ were 0.1812, 0.1896, and 5.7737 a.u., respectively.

Molecular Electrostatic Potential (MEP)
One way of determining the electrostatic potential values over the iso-electronic density map is to investigate a three-dimensional (3D) layout of the molecular electrostatic potential (MEP) surface. The MEP is conducted for the estimation of electrophilic and nucleophilic attacks on chemical systems [54]. The MEP diagram shows a variety of colors, red, blue, yellow, green, light blue, and blue, which represent significantly electron-rich, slightly electron-rich, neutral, slightly electron-deficient, and significantly electron-deficient regions, respectively [55]. The morphology, molecular size, and electrostatic potential amplitude of the PESMP compound are all clearly shown in Figure 10. In the PESMP compound, the charge density for HOMO was found over the oxadiazole and benzenesulfonamide moieties (Figure 9). The charge density for LUMO was situated on the phthalimide moiety, predicting an excellent charge transference from oxadiazole and benzenesulfonamide toward the phthalimide moiety.
The chemical hardness (η) of a molecule is related to the energy gap (ΔE) value. The overall softness and reactivity of the PESMP compound demonstrated an inverse relationship. η showed a value of 0.0866 a.u., revealing the high stability and lower reactivity of the considered compound. The ionization potential (IP) and electron affinity (EA) values were 0.2678 and 0.0946 a.u., respectively. Moreover, the values of µ, ω, and σ were 0.1812, 0.1896, and 5.7737 a.u., respectively.

Molecular Electrostatic Potential (MEP)
One way of determining the electrostatic potential values over the iso-electronic density map is to investigate a three-dimensional (3D) layout of the molecular electrostatic potential (MEP) surface. The MEP is conducted for the estimation of electrophilic and nucleophilic attacks on chemical systems [54]. The MEP diagram shows a variety of colors, red, blue, yellow, green, light blue, and blue, which represent significantly electron-rich, slightly electron-rich, neutral, slightly electron-deficient, and significantly electron-deficient regions, respectively [55]. The morphology, molecular size, and electrostatic potential amplitude of the PESMP compound are all clearly shown in Figure 10. In the MEP map of the PESMP compound displayed in Figure 10, a red-colored zone is noted around the oxygen atoms. The likelihood of an electrophilic attack is therefore related to this area, which represents the electron-rich zone. On the hydrogen and certain carbon atoms, green and blue zones are seen, signifying electron-deficient zones, which point to a nucleophilic attack on these potential sites.

α-Amylase Inhibition Activity
The inhibitory potential of a probenecid-derived 1,3,4-oxadiazole-phthalimide hybrid (PESMP) against α-amylase was investigated at concentration levels ranging from 10 to 200 μg/mL, with PESMP inhibiting α-amylase by 81.06% at 200 μg/mL (Table 5). Acarbose, a commercially used standard α-amylase inhibitor, demonstrated inhibitory activity with an IC50 value of 8.80 ±0.21 μg/mL. In the MEP map of the PESMP compound displayed in Figure 10, a red-colored zone is noted around the oxygen atoms. The likelihood of an electrophilic attack is therefore related to this area, which represents the electron-rich zone. On the hydrogen and certain carbon atoms, green and blue zones are seen, signifying electron-deficient zones, which point to a nucleophilic attack on these potential sites.

Molecular Docking
The efficiency of the AutoDock4.2.6 package in anticipating the correct inhibitor-αamylase binding pose was validated. For validation purposes, the co-crystallized acarbose ligand was re-docked in the α-amylase enzyme's active site, and the anticipated docking pose was compared to the experimental binding mode (PDB ID: 1ose [56]) ( Figure S5). From Figure S5, the predicted docking pose was similar to the binding mode of the native structure of the acarbose inhibitor with an RMSD value of 0.23 Å, exhibiting several hydrogen bonds with the key amino acid residues of the α-amylase enzyme [25].
The docking score and pose of PESMP against the α-amylase enzyme were predicted and compared to that of acarbose with the aid of AutoDock4.2.6. The anticipated docking score and pose are presented in Figure 11.

Molecular Docking
The efficiency of the AutoDock4.2.6 package in anticipating the correct inhibitor-αamylase binding pose was validated. For validation purposes, the co-crystallized acarbose ligand was re-docked in the α-amylase enzyme's active site, and the anticipated docking pose was compared to the experimental binding mode (PDB ID: 1ose [56]) ( Figure S5). From Figure S5, the predicted docking pose was similar to the binding mode of the native structure of the acarbose inhibitor with an RMSD value of 0.23 Å, exhibiting several hydrogen bonds with the key amino acid residues of the α-amylase enzyme [25].
The docking score and pose of PESMP against the α-amylase enzyme were predicted and compared to that of acarbose with the aid of AutoDock4.2.6. The anticipated docking score and pose are presented in Figure 11.  As depicted in Figure 11, PESMP demonstrated a −7.4 kcal/mol docking score. The potency of PESMP as an α-amylase inhibitor may be relevant to its ability to form a hydrogen bond with HIS305 (2.07 Å). Moreover, PESMP exhibited π· · · π T-shaped and π· · · π stacked interactions with the TYR62 residue and a π-anion interaction with the ASP197 residue. Moreover, PESMP demonstrated a carbon-hydrogen bond with the TRP59, TYR151, and GLY306 residues, a π-alkyl interaction with the VAL163 and ALA198 residues, and alkyl interactions with the LYS200, HIS201, and ILE235 residues (Figure 11).

Experimental Details
The current work was supported by the use of easily available laboratory-grade chemicals and reagents. The utilized solvents were of analytical grade and were employed without drying or distillation. The melting point was measured in an open capillary using a Gallenkamp melting point device (MP-D). Thin-layer chromatography was used to monitor all reactions using Merck pre-coated plates (silica gel 60 F254, 0.25 mm). Using UV rays (254 nm), fluorescence quenching was adopted to view the results. A Bruker AV-300 (300 MHz) spectrometer was employed to record the 1 H and 13 C NMR spectra. Singlecrystal X-ray diffraction data were collected for PESMP compound on Bruker Kappa APEX-II CCD diffractometer with molybdenum X-ray source, which generated k α radiations with a wavelength value of 0.71073 Å. The structure was solved and refined by SHELXT-2014 [57] and SHELXL-2019/2 [58], respectively. Mercury version 4.0 software [59] and PLATON [60] were employed for graphically illustrating single-crystal X-ray diffraction results. A modified multistep synthetic procedure was followed to access PESMP.
Step I: In a typical experimental procedure, probenecid (PE) (30 mmol) was esterified in 20 mL of methanol using catalytic amounts of sulfuric acid (0.5 mL) at reflux temperature for 4 h. The mixture was extracted thrice with 30 mL of ethyl acetate after being neutralized with 50 mL of saturated sodium bicarbonate solution. The organic layer was dried over anhydrous sodium sulphate and filtered, and then the solvent was removed to obtain crude methyl ester of probenecid in a quantitative yield.
Step II: Methyl ester of probenecid (MPE) (with 25 mmol) was dissolved in 30 mL of methanol, and NH 2 NH 2 .H 2 O (80%, 0.06 mol) was added dropwise. After refluxing for 8 h, the reaction mixture was cooled to 25 • C and then dispensed into ice-cold water. Probenecid hydrazide (PEH) was precipitated, filtered, dried, and finally recrystallized from MeOH.
Step III: A solution of probenecid hydrazide (PEH) (20 mmol) in 10 mL of methanol and 3 equivalents of KOH dissolved methanol (30 mL) were added. After 10 min, carbon disulfide (30 mmol) was slowly added. Afterwards, the reaction mixture was refluxed for about 12 h. The reaction mixture was cooled down to 25 • C, concentrated, and poured into ice-cold water. The solution was acidified (pH = 2) with dilute hydrochloric acid. The precipitated probenecid oxadiazole (PEO) was washed with warm water and purified by recrystallization with the help of MeOH.
Step IV: Probenecid oxadiazole (PEO) (10 mmol) was dissolved in acetone and 12 mmol of potassium carbonate was added. After stirring for 10 min at 25 • C, 12 mmol of N-(bromomethyl)phthalimide was added, and the reaction mixture was stirred for another 6 h. The solvent was removed, and the crude was recrystallized from methanol to obtain pure PESMP (Scheme 1).

Hirshfeld Surface (HS) Analysis
Hirshfeld surface (HS) was analyzed for PESMP compound using CrystalExplorer version 21.5 [61] to further elucidate features of non-covalent interactions within a single crystal. In that spirit, the surface of normalized contact distance (d norm ) was extracted using a color range from −0.2450 to 1.5592 a.u. Moreover, a map of the shape index property was generated with a color scope ranging from −1.0 a.u. (concave) to 1.0 au (convex). Two-dimensional fingerprints were created to unveil the contribution of interatomic contact to the overall crystal packing. To investigate the crystal packing environment widely, the enrichment ratio was evaluated by dividing the actual contact by the random contact theoretical proportion. Voids were also divulged using the Hartree-Fock theory to understand the properties of the single crystal from a mechanical point of view. Energy framework computations were performed to illustrate the energy framework and interaction energies of PESMP compound. Interaction energy calculations were carried out on a cluster of molecules located within 3.8 Å 3 of the reference molecule using the B3LYP method with a 6-31G(d,p) basis set.

Density Functional Theory (DFT) Analysis
DFT-based computations were performed with the Gaussian 09 program package [62] in conjugation with M06/6-311G(d,p) function for the quantum chemical investigations of synthesized PESMP compound. The input files were developed by using the GaussView 6.0 program [63]. To demonstrate the contributions of the electron density surrounding the molecular orbitals, FMOs theory was invoked. The distributions of HOMO and LUMO were generated. Using FMOs, energies of HOMO (E HOMO ) and LUMO (E LUMO ) were computed for the PESMP compound. Band gaps were accordingly assessed as the difference between the energies of LUMO and HOMO levels, as shown in the following Equation (1): Several global reactivity parameters (GRPs) were calculated for the PESMP compound as per Equations (2)-(8): MEP plot was generated for pictorially addressing the chemical nature of the PESMP compound. In MEP map, blue, green, yellow, orange, and red represented regions with decreasing order of positive electrostatic potential magnitudes.

Enzyme Inhibition Activity
α-Amylase inhibition potential of probenecid-derived 1,3,4-oxadiazole-phthalimide hybrid (PESMP) was investigated employing the 3,5-dinitro-2-hydroxybenzoic acid (DNS) method [64]. PESMP (1 mg) and DNS (1 mg) were separately solvated in 1 mL of DMSO. A solution of PESMP and α-amylase (200 µL, pH 7.0) was maintained at 30 • C for 10 min. An aqueous starch solution (1%) was poured and the same temperature was regulated for another 3 min. The reaction was stopped by adding a DNS reagent (200 µL). The tube was immersed in boiling water. After 10 min, the tube was cooled down to 25 • C, and distilled water (5 mL) was added. The absorbance was obtained at 540 nm. Acarbose (10-250 µg/mL) was utilized as a standard inhibitor for the comparison of the inhibitory potential of PESMP in triplicate experiments, whereas 2% DMSO was used for the control incubation, which represents maximal enzyme activity. Percentage inhibition was calculated by using a formula (Equation (9)), and then IC 50 values were calculated. % α amylase inhibition = Ao − Ai Ao × 100 (9)

Molecular Docking
The employed docking calculations are detailedly described elsewhere [65][66][67]. Briefly, the α-amylase crystal structure (PDB access code: 1ose [56]) complexed with acarbose was retrieved and employed as a template for docking predictions. For the purpose of preparation, all ions, heteroatoms, and crystallographic water molecules were eliminated. The protonation states of the α-amylase enzyme were scrutinized with the assistance of the H++ website [68]. In addition, all missing hydrogens were added. The structure of PESMP was manually built, and then energetically minimized using MMFF94S force field within SZYBKI software [69,70]. The Gasteiger method was utilized to assign the atomic charges of PESMP and acarbose compound [71]. In this work, docking computation was conducted utilizing AutoDock4.2.6 software [72]. The genetic algorithm number (GA) was adjusted to 250. The maximum number of energy evaluations (eval) was set to 25,000,000. Other docking parameters were set to default values. The grid box was tailored to involve the binding pocket of the α-amylase enzyme, with a grid size of 60 Å × 60 Å × 60 Å. The coordinates of the grid center were x = 32.644, y = 38.464, and z = −3.166. The AutoGrid program was employed to extract the grid maps with a spacing of 0.375 Å. All molecular interactions were represented using BIOVIA Materials Studio [73].

Conclusions
An efficient, multistep synthetic approach was followed to synthesize good yields of 4-(5-((1,3-dioxoisoindolin-2-yl)methylthio)-1,3,4-oxadiazol-2-yl)-N,N-dipropylbenzenesulfonamide (PESMP). Its synthesis was confirmed via structural validation using NMR ( 1 H, 13 C), FT-IR, and single-crystal X-ray diffraction analyses. The purity of PESMP was established on the basis of thin-layer chromatography. To obtain further insight into the features of the entitled compound, various DFT calculations were executed accordingly. The band gap value of the PESMP compound (0.1732 a.u.) for the HOMO-LUMO orbital was smaller than the band gap values of HOMO-LUMO ±1 and HOMO-LUMO ±2. The testing of PESMP against α-amylase revealed an IC 50 = 10.60 ±0.16 µg/mL using acarbose (IC 50 = 8.80 ±0.21 µg/mL) as a standard drug. Molecular docking revealed the binding mode of the PESMP compound against the active site of α-amylase. PESMP and acarbose showed docking scores of −7.4 and −9.4 kcal/mol against the α-amylase enzyme, respectively. These findings shine new light on the potential of the PESMP compound as an α-amylase inhibitor.
Supplementary Materials: The following supporting information can be downloaded at: https: //www.mdpi.com/article/10.3390/ph16030424/s1, Figure S1: 1 H NMR spectrum of PESMP; Figure  S2: 13 C NMR spectrum of PESMP; Figure S3: 2D fingerprint plots of the remaining contacts; Figure  S4: Graphical representation of voids, (a) 1st view, and (b) 2nd view along the a-axis; Figure S5: 3D superimposition of the resolved experimental structure (in gray) and the portended binding mode (in cyan) of acarbose complexed with α-amylase enzyme; Table S1: Selected bond lengths and bond angles in the PESMP compound; Table S2: Interaction energies (kJ/mol); Table S3: Cartesian coordinates of the selected atoms that are involved in interaction energy calculations.